Determine the pH of a solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 3 NEXT > A solution is prepared with 0.075 M (CH3)³N and 0.10 M (CH3)NHCI. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -2x 0.10-2x (CH3)3N(aq) + 0 0.075 + x 0.075 0.075-x 0.10 2 H₂O(l) 0.075 + 2x 5.2 x 10- 0.075 - 2x +x OH (aq) 0.10 + x -X 0.10-x + (CH,),NH*(aq) RESET +2x 0.10+2x
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- ermine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. 2 NEXT > Two solutions are mixed: 40.0 mL of 0.500 M NH, and 25.0 mL of 0.300 M HCI. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base.. NH3(aq) NH, (aq) (be),H Before (mol) Change (mol) After (mol) 5 RESET 40.0 0.500 25.0 0.300 0.300 -x 0.0075 -0.0075 0.0100 -0.0100 0.0125 -0.0125 0.0200 -0.0200 Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. NH3(aq) H,O(1) OH (aq) NH, (aq) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.500 0.300 0.192 0.313 0.115 0.500 -x 0.300 -x 0.192 +* 0.192 -x 0.500 + x 0.300 +x 0.313 + x 0.313 -x 0.115 +x 0.115-xDetermine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. NEXT > The buffer was prepared by dissolving 21.5 g HC,H,O₂ and 37.7 g of NaC,H,O₂ in 200.0 mL of solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) 0.178 0.880-x [0] [0.888] [1.31 + x) 0 0 0.888 1.31 + x HC₂H5O₂(aq) + [21.5] [x] Ka = 4.2 x 10-² 21.5 0.178 + x +x [37.7] [2x] 1 [0.178+x][0.888 + x] 37.7 -x 0.888 + x Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 6.23 The Ka for HC₂H5O₂ is 6.3 x 10-5. Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka…Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Kb = = 5.2 × 10-4 RESET [0] [0.075] [0.10] [5.2 × 10] [x] [2x] [2x]² [0.075 + x] [0.075 - x] [0.075 + 2x] [0.075 - 2x] [0.10+x] [0.10 - x] [0.10 + 2x] [0.10 -2x] < PREV 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the pH of the solution. pH = RESET 0 7.86 6.14 0.075 3.9 × 10 3.41 10.59 1.12
- Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 3 > A solution is prepared with 0.55 M HNO2 and 0.75 M KNO2. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -2x 0.75 -2x 0 1 HNO₂(aq) 0.55 + x 0.55 -X 0.55-x 0.55 0.55 - x 0.75 2 H₂O(l) III 0.55 + 2x 6.8 x 104 0.55 - 2x 1L +x H3O+(aq) 0.75 + x +x -X 0.75-x + NO₂ (aq) RESET +2x NEXT 0.75 + 2x +xA solution is prepared that is initially 0.078M in propanoic acid (HC,H,CO,) and 0.38M in potassium propanoate (KC,H,CO,). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in H30" |. You can leave out the M symbol for molarity. [HC,H,Co,] [c,,co] [1,0] initial change finalA solution is prepared that is initially 0.30M in hydrofluoric acid (HF) and 0.13M in potassium fluoride (KF). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [H3O+]. You can leave out the M symbol for molarity. [HF] [F] [H,O] initial 0 0 change 0 final 0 0 ㅁ 1 G
- 0.0500 M HF (Ka= 7.20 x 10–4) determine the equilibrium molar concentration of H3O+ and equilibrium molar concentration of HF (in 3 sig. figures).Determine the Kb for a base by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. Initial (M) Change (M) Equilibrium (M) NEXT The pH for a 0.0160 M solution of CH3C6H4NH₂ is 8.600. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. -2.50 × 10-9 1 CH3C6H4NH₂(aq) + 0 3.98 x 10-6 0.0160 -3.98 x 10-6 8.60 5.4 H₂O(1) -8.60 -5.4 2 = OH-(aq) 0.93 -0.93 + CH3C6H4NH3 + (aq) RESET 2.50 × 10-9Determine the pOH of a weak acid (HA) solution by constructing an ICE table and using this information to determine the pOH of the solution. Complete Parts 1-2 before submitting your answer. 1 A 0.200 M aqueous solution of HA is 3.0% dissociated at equilibrium. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) HA(aq) + H₂O(l) 2 H3O+ (aq) 2 NEXT > + A-(aq)
- Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 3 NEXT > The buffer was prepared by dissolving 21.5 g HC7H5O2 and 37.7 g of NaC7H5O₂ in 200.0 mL of solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) 0.178 0.880 - x 0 0.888 1 HC7H5O₂(aq) + 1.31 + x 21.5 +X 0.178 + x 37.7 -X H₂O(1) 0.888 + x 0.176 21.5-x H3O+ (aq) 0.261 37.7 + x + 0.880 0.176 - x C7H5O₂ (aq) RESET 1.31 0.261 + xA solution is prepared that is initially 0.26M in hydrofluoric acid (HF) and 0.25M in potassium fluoride (KF). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [H₂O*]. You can leave out the M symbol for molarity. initial change final [HF] 0 П [F] 0 0 0 [H₂O*] 0 0 0 XDetermine the pH of a solution of HF by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Ka of HF is 6.8 x 10-4. Complete Parts 1-3 before submitting your answer. NEXT > A 0.30 M aqueous solution of HF is prepared. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -2x 6.8 x 10-4-2x 0 0.30 + x 1 HF(aq) 0.30 0.30 - x + H₂O(l) 6.8 x 10-4 2 0.30 + 2x 0.15 0.30 - 2x H3O+(aq) + +X 3 6.8 x 104 + x -X 6.8 x 10-4-x F-(aq) ✓ RESET +2x 6.8 x 10-4 + 2x